Textbook Question
(b) Use the energy requirements of these two pro- cesses to explain why photodissociation of oxygen is more important than photoionization of oxygen at altitudes below about 90 km.
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Ch.18 - Chemistry of the Environment
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 18, Problem 17b
The dissociation energy of a carbon-bromine bond is typically about 276 kJ/mol. (b) Which kind of electromagnetic radiation—ultraviolet, visible, or infrared—does the wavelength you calculated in part (a) correspond to?
Verified step by step guidance1
First, understand that the dissociation energy given (276 kJ/mol) is the energy required to break one mole of carbon-bromine bonds.
Convert the dissociation energy from kJ/mol to J/photon. Since 1 kJ = 1000 J, multiply 276 kJ/mol by 1000 to convert to J/mol, then divide by Avogadro's number (6.022 x 10^23 mol^-1) to find the energy per photon.
Use the energy of a photon equation: E = h * c / λ, where E is the energy per photon, h is Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength in meters.
Rearrange the equation to solve for wavelength (λ): λ = h * c / E. Substitute the values for h, c, and the energy per photon calculated in the previous step to find the wavelength.
Compare the calculated wavelength to the typical ranges of electromagnetic radiation: ultraviolet (10 nm to 400 nm), visible (400 nm to 700 nm), and infrared (700 nm to 1 mm) to determine which type of radiation corresponds to the calculated wavelength.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Dissociation Energy
Dissociation energy is the amount of energy required to break a bond between two atoms in a molecule, resulting in the formation of separate atoms. In this case, the dissociation energy of the carbon-bromine bond is 276 kJ/mol, indicating the energy needed to separate carbon and bromine atoms. Understanding this concept is crucial for relating energy changes to electromagnetic radiation.
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Electromagnetic Radiation
Electromagnetic radiation encompasses a range of waves, including ultraviolet, visible, and infrared light, characterized by their wavelength and energy. Each type of radiation corresponds to specific energy levels, with ultraviolet having higher energy and shorter wavelengths, while infrared has lower energy and longer wavelengths. This concept is essential for determining which type of radiation is associated with the energy calculated from the dissociation energy.
Wavelength and Energy Relationship
The relationship between wavelength and energy is described by the equation E = hc/λ, where E is energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. This equation shows that shorter wavelengths correspond to higher energy photons, while longer wavelengths correspond to lower energy. Understanding this relationship is key to identifying the type of electromagnetic radiation based on the energy derived from the dissociation energy.
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Related Practice
Textbook Question
From the data in Table 18.1, calculate the partial pressures of carbon dioxide and argon when the total atmospheric pressure is 1.05 bar.
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Textbook Question
(a) Distinguish between photodissociation and photoionization.
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Textbook Question
The dissociation energy of a carbon-bromine bond is typically about 276 kJ/mol. (a) What is the maximum wavelength of photons that can cause C-Br bond dissociation?
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Textbook Question
The wavelength at which the O2 molecule most strongly absorbs light is approximately 145 nm. (a) In which region of the electromagnetic spectrum does this light fall?
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